My Notes O Ask Your 1. -1 points OSGenChem1 5.3.WA.001 Industrial production of

Question

My Notes O Ask Your 1. -1 points OSGenChem1 5.3.WA.001 Industrial production of nitric acid, which is used in many products including fertilizers and explosives, approaches 10 billion kg per year worldwide. The first step in its production is the exothermic axidation of ammonia, represented by the following equation. 4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g) If this reaction is carried out using 7.112x103 g NH3 as the limiting reactant, what is the change in enthalpy? k) Supporting Materials constants and Factors Periodic Table Supplemental Data Additional Materials Section 5.3 Tutorial 2. ·-1 points 15.3 WA 008 My Notes Ask Your Calculate the standard enthalpy change (AH n) for the reaction of TICI4(0) and H 0(g) to form TIO2(s) and HK@) given the standard enthalples of formation (AH ) shown in the table below. (tnclude the sign of the value in your answer) 12 kJ Compound ,(k /mol) TICI4(g) H20(g)241.8 TIO2(s) HCI(g) -763.2 944.0 -92.3

Explanation / Answer

Q1.

change to moles of NH3

mol = mass/MW = (7.112*10^3)/17 = 7112 mol of NH3

1 mol of NH3 = -902 kJ released

7112 mol of NH3 = x

x = 7112*902

x = 6415024 kJ of heat released (negative)

Q2

first, balance reaction

TiCl4 + H2O = TiO2 + HCl

TiCl4 + 2H2O = TiO2 + 4HCl

HRxn = Hproducts -Hreactants

HRXN = TiO2 + 4HCl - (TiCl4 + 2H2O)

HRxn = -944 + 4*-92.3 - (-763.2 + 2*-241.8)

HRXN = -66.4 kJ/mol

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